Transcript chapter 1 - Columbia University

Standards for Measurement
Preparation for College Chemistry
Columbia University
Department of Chemistry
The Scientific Method
Observations
(analysis)
Laws
Hypothesis
(explanation)
Experiment
(measurement)
(analysis)
Theory
(Model)
Measurement and Interpretations
Direct Measurement
Diameter = 2.5 cm
1
2
3
4
5
6
7
8
Interpretation Step
Radius = Diameter/2
Area =  x r2 = 8.04 cm2
Art of Scientific Measurement:
• Recognize what can be measured directly.
• Devise a way to obtain the desired information from measurement data.
Experimentation
Measured Data
Basic
UNIT
Resting Potential = -65 mV
Derived
Affected by Uncertainty
• Accuracy
NUMERICAL VALUE
• Precision
• Resolution
• Noise
Significant Figures (Sig. Figs.)
The mass of an object weighed on a triple beam balance
(precision ± 0.1g) is found to be 23.6 g.
This quantity contains 3 significant figures, i.e., three
experimentally meaningful digits.
If the same measurement is made with an analytical balance
(precision ± 0.0001g) , the mass might be 23.5820 g (6 sig.
fig.)
Evaluating Zero
Zero is SIGNIFICANT when:
Is between nonzero digits: 61.09 has four sig Figs.
Appears at the end of a number that includes a decimal point 0.500 has
three sig. Figs.; 1000. has four sig. Figs.
Zero is NON SIGNIFICANT when:
Appears before the first nonzero digit. 0.0025 has two sig. Figs. Leading
Zeros are non significant
Appears at the end of a number without a decimal point. 1,000 has
one sig. Fig.; 590 has two sig. Figs.
Exact Numbers
Defined numbers, like 12 inches in a foot, 60 minutes in an hour,
1,000mL in one liter.
Numbers that occur in counting operations.
Exact numbers have an infinite number of sig. figs.
Exact numbers do not limit the number of sig. figs. in a calculation.
Scientific Notation
Number written as a factor between 1 and 10 multiplied by
10 raised to a power.
0.0468  4.68  10 2
0.00003  3.0 10 5 (two digits)
or 3 10 5 (one digit)
Useful to unequivocally designate the significant figures.
1200  1.200  10 3 (four digits)
6,600, 000  6.6 10 6 (two digits)
Multiplication or Division
The answer must contain as many significant figures as in the
least precise quantity (measurement with least precision).
What is the density of a piece of metal weighing 36.123 g
with a volume of 13.4 mL?
Drop these three digits
mass
36.123g
d

 2.69575g / mL
volume 13.4mL
Round off to 7
ANSWER:
2.70g / mL
Addition or Subtraction
Keep only as many digits after the decimal point as there are
in the least precise quantity
Ex. Add 1.223 g of sugar to 154.5 g of coffee:
Total mass = 1.2 g + 154.5 g = 155.7 g
Addition or Subtraction
Note that the rule for addition and subtraction does not relate to
significant figures.
The number of significant figures often decreases upon subtraction.
Mass beaker + sample = 52.169 g
(5 sig. figs.)
- Mass empty beaker = 52.120 g
(5 sig. figs.)
Mass sample = 0.049 g
(2 sig figs)
SI Units Prefixes (Multiples)
Prefix
Symbol
Value
Power
exa
E
1,000,000,000,000,000,000 1018
peta
P
1,000,000,000,000,000
1015
tera
T
1,000,000,000,000,
1012
giga
G
1,000,000,000
109
mega
M
1,000,000
106
kilo
k
1,000
103
hecto
h
100
102
deka
da
10
101
SI Units Prefixes (Submultiples)
Prefix
Symbol
Value
Power
atto
a
0.000000000000000001
10-18
femto
f
0.000000000000001
10-15
pico
p
0.000000000001
10-12
nano
n
0.000000001
10-9
micro
µ
0.000001
10-6
milli
m
0.001
10-3
centi
c
0.01
10-2
deci
d
0.1
10-1
Système International (SI)
The Metric System
Physical Quantity
Name
Symbol
Length
Mass
Time
Electric current
Temperature
Amount of substance
Luminous intensity
meter
kilogram
second
ampere
kelvin
mole
candela
m
kg
s
A
K
mol
cd
Based on seven DIMENSIONALLY INDEPENDENT quantities
Length
Base unit is the meter (m)
1790s: 10-millionth of the distance from the equator to
the North Pole along a meridian.
1889: Distance between two engraved lines on a PlatinumIridium alloy bar maintained at 0°C in Sevres-France.
1960-1983: 1,650,763.73 wavelengths of the orange-red
emision of 18Kr at standard conditions
Since 1983: 1/299,792,458 of the distance traveled by
light in 1 second through vacuum.
Length
Engineering dimensions
1 km = 103 m
1 in = 2.54cm
1 cm = 10-2 m
1 mile = 1.61km
1 mm = 10-3 m
1 µm = 10-6 m
Atomic dimensions
1 nm = 10-9 m
1 Å = 10-10 m
Mass
Base unit is the kilogram (kg)
International prototype: a platinum-iridium cylinder
maintained in Sevres-France.
1 kg = 103 g; 1 mg = 10-3 g
A mass of 1 kg has a terrestrial weight of 9.8 newtons (2.2 lbs)
Depending on the precision required and the amount of
material, different balances are used:

The Quadruple Beam Balance (± 10 mg)

The Top Loading Balance (± 1 mg).

The Analytical Balance (± 0.1 mg).
Comparison of Temperature Scales
°F = (1.8 x °C ) + 32
Fahrenheit
K = °C + 273.15
°C = (°F - 32) / 1.8
Kelvin
Celsius
212
100
Freezing point of water
32
0
373.15
100
Boiling point of water
273.15
Temperature Conversion
K = °C + 273.15
°F = (1.8 x °C ) + 32
°C = (°F - 32) / 1.8
Ex. 2.20 Convert 110°F to °C and K
°C = (68° – 32°) / 1.8 = 20°C
K = 20 + 273 = 293 K
Derived Units
Physical quantity
Name
Symbol
Definition
Frequency
Force
Pressure, stress
Energy work, heat
Electric charge
Electromotive Force
Electric Resistance
Hertz
newton
pascal
joule
coulomb
volt
ohm
Hz
N
Pa
J
C
V

s-1
m.kg.s-2
N.m-2 = m-1.kg.s-2
N.m = m2.kg.s-2
A.s
J.C-1 = m2.kg.s-3. A-1
V.A-1 = m2.kg.s-3. A-2
Measurement of Volume
Conversion Factors
2.54cm
1 in
1 in  2,54cm 
or
1 in
2.54cm
Two conversion factors
Unit needed
 Unit needed
Unit given 
Unit given
Dimensional Analysis
•Read Problem. What needs to be solved for? Write it down
•Tabulate data given. Label all factors with proper units
•Determine principles involved and unit relationships
•Set up the problem deciding for the proper conversion factor
•Perform mathematical operations
•Check if the answer is reasonable
Simple, One Step Conversions
CBS News reported the barometric pressure to be 99.6 kPa.
Express this in mm Hg.
Conversion factor : 101.3 kPa = 760 mm Hg
Unit needed
pressure (mmHg) = 99.6kPa x 760 mm Hg = 747mmHg
101.3 kPa
Unit given
Unit given
Simple, One Step Conversions
A rainbow trout is measured to be 16.2 in. long. What is the
length in cm?
length in cm = 16.2 in x
2.54 cm
= 41.1 cm
1 in
Note the cancellation of units. To convert from centimeters
to inches, the conversion factor would be 1 in / 2.54 cm.
Multiple Conversion Factors
A baseball is thrown at 89.6 miles per hour. What is the speed
in meters per second?
Mile/hour
m/hour
m/s
1 mile = 1.609 km = 1.609 x 10-3 m; 1 h = 3600 s
1h
miles x 1.609 x 10–3m
= 40.0 m / s
speed = 89.6
x
1 mile
3600 s
hour
Three sig. figs.
Units raised to a Power
The conversion factor must also be raised to that power.
A circle has an area of 28 in2. Calculate area in cm2.
in2
cm2
(1 in)2 = (2.54 cm)2
2
(2.54
cm)
2
Area = 28 in x
(1 in)2
6.45 cm2
2 cm2
=
1.8
x
10
=
1 in2
Two sig. figs.
Density: Conversion factor
mass
volume
An empty flask weighs 22.138 g. You pipet 5.00 mL of octane into
the flask. The total mass is 25.598 g. What is the density?
Octane amount in g:
25.598
-22.138
3.460g
3.460g
d=
= 0.692g / mL
5.00 mL
What is the volume occupied by ten grams of octane?
V = 10.00g x
1 mL
0.692g
= 14.5 mL
Solubility
Expressed as grams of solute per 100 g of solvent in the
CRC (Chemical Rubber Company) Chemistry and Physics
Handbook.
For lead nitrate in aqueous solution:
Solubility (g/100g water)
T (°C)
50
10
140
100
Solubility
How much water is required to dissolve 80 g of lead nitrate
at 100°C?
100g water
Mass water = 80g lead nitrate x
= 57g water
140g lead nitrate
Conversion factor
(from table)
Cool the solution to 10°C. How much lead nitrate remains in
solution?
50g lead nitrate
Mass of lead nitrate = 57g water x
100g water
= 28g lead nitrate
28g lead nitrate remain in solution
80g lead nitrate were initially in solution
80g – 28g = 52g lead nitrate crystallizes out of solution